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(B) The total number of electrons in $O_{2}^{2-}$ is $8 + 8 + 2 = 18$.The molecular orbital configuration is: $\sigma_{1s}^{2} \sigma_{1s}^{*2} \sigma

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(B) The total number of electrons in $O_{2}^{2-}$ is $8 + 8 + 2 = 18$.The molecular orbital configuration is: $\sigma_{1s}^{2} \sigma_{1s}^{*2} \sigma_{2s}^{2} \sigma_{2s}^{*2} \sigma_{2p_{z}}^{2} (\pi 2p_{x}^{2} = \pi 2p_{y}^{2}) (\pi_{2p_{x}}^{*2} = \pi_{2p_{y}}^{*2})$.Since all molecular orbitals are completely filled,there are $0$ unpaired electrons.

According to molecular orbital theory,the number of unpaired electron$(s)$ in $O_{2}^{2-}$ is :

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